Science Decisions Involving Thermochemistry/Enthalpy Changes/ Experimentation in thermochemistry/Bonding and Hess's Law
NB Prescribed Outcomes
describe the importance of peer review in the development of your knowledge about thermochemistry. (114-5)
use library and electronic research tools to collect information on a given topic. (213-6)
select and integrate information from various print and electronic sources or from several parts of the same source. (213-7)
identify multiple perspectives that influence a science-related decision or issue involving thermochemistry. (215-4)
define endothermic reaction, exothermic reaction, specific heat capacity, enthalpy, bond energy, heat of reaction, and molar enthalpy. (324-2)
define thermochemistry and thermodynamics.
differentiate between endothermic and exothermic changes.
calculate specific heat capacity.
use specific heat capacity in calculations.
perform heat transfer problem
illustrate changes in energy of various chemical reactions, using potential energy diagrams. (324-5)
dentify exothermic and endothermic processes from the sign of Δ, from thermochemical equations, and from labeled enthalpy/ potential energy diagrams.
label enthalpy diagrams given either the Δ for a process or a thermochemical equation.
compile and display evidence and information on heats of formation in a variety of formats, including diagrams, flow charts, tables, and graphs. (214-3)
write thermochemical equations including the quantity of energy exchanged given either the value of Δ or a labeled enthalpy diagram, and vice versa
compare the molar enthalpies of several combustion reactions involving organic compounds. (324-7)
write and balance chemical equations for combustion reactions of alkanes, including energy amounts. (324-1)
calculate and compare the energy involved in chemical reactions. (324-3)
calculate the changes in energy of various chemical reactions using bond energy, heats of formation, and Hess’s Law (324-4)
apply one of the methods of predicting heats of reactions to your experimentally determined lab values (214-6)
- conduct a Hess’s Law experiment
compare experimental results to theoretical calculations from heat of formation or bond energy data
analyse and describe examples where technologies were developed based on understanding thermochemistry (116-4)
Students will be expected to
work cooperatively with team members to develop and carry out thermochemistry experiments (215-6)
evaluate and select appropriate instruments for collecting evidence and appropriate processes for problem solving and inquiring (212-8)
design a thermochemistry experiment identifying and controlling major variables (212-3)
determine experimentally the changes in energy of various chemical reactions (324-6)
analyse the knowledge and skills acquired in their study of thermochemistry to identify areas of further study related to science and technology (117-9)
- compare physical, chemical, and nuclear changes in terms of the species and the magnitude of energy changes involved
propose alternative solutions to solving energy problems and identify the potential strengths and weaknesses of each (214-15)
-
explain, in simple terms, the energy changes of bond breaking and bond formatio
calculate the heat gained or lost from a system using the thermochemical equatio
Ch 22, 23 Organic Chemistry
CHEM 122
Outcomes
Essential Questions
Unit 1: Thermochemistry (23 hours) 1) Introduction to Thermochemistry (4 hrs) The relevance of thermochemistry is introduced with the investigation of calorimetry to analyze food products. Alternative fuel energies are investigated with respect to non fossil-fuel combustion. -Thermochemistry STSE -Science Decisions 2) Enthalpy (14 hrs) Identify and calculate energy changes associated with phase changes. The construction of heat curves and the analysis of its individual components are explored both qualitatively and quantitatively. A lab reinforces this concept through construction of a basic calorimeter. “Heat Capacity of Calorimeter” “Heat of Reaction” “Specific Heat of a Metal” -Enthalpy Changes -Thermochemistry Experimentation 3) Bonding and Hess’ Law (5 hrs) Theoretical enthalpy is calculated using Hess’ law for instances where practical applications cannot be applied. 117-6,118-2, 118-8,118-10, 114-5, 213-6, 213-7, 215-4, 324-2,324-5, 214-3, 324-7, 324-1, 324-3, 215-6,212-8 ,212-3, 324-6, 117-9, 214-15, 324-4, 214-6, 116-4
Unit 2: From Solutions to Kinetics to Equilibrium (15 hours)
1) Kinetics and Rate of Reaction (3 hrs) Factors affecting the rates of reaction relating to kinetics are investigated. 2) Collision Theory, Reaction Mechanisms and Catalysts (3 hrs) Collision theory and Le Châtelier’s principle are used in predicting the direction of reactions. 3) Chemical Equilibrium (9 hrs) Calculating equilibrium constants is used in predicting the direction of reactions.
Unit 3: Acids and Bases (23 hours) 1) Properties and Definitions of Acids and Bases (4 hrs) Using various models (Arrhenius, and Brønsted-Lowry), students learn the various characteristics, properties and behaviors of acids and bases. The limitations of the Arrhenius Theory are identified. Individual ion concentrations are calculated based on dissociation equations. 2) Acid/Base Reactions (4 hrs) The Brønsted-Lowry Theory is explored in detail. Acids, bases, conjugate acid-base pairs and amphoteric substances are identified. Students learn to predict the products of acid-base reactions by using a table of acid-base strengths. 3) OH-, H3O and Le Châtelier (3 hrs) The self-ionization of water and Kw is introduced. Illustrate the use of indicators and Le Chateliers Principle in action. 4) Using the Equilibrium Concept with Acids and Bases (7 hrs) Perform calculations of pH, pOH, and so on using Kw. Identify strong acids and bases. Identify weak acids and bases, define % dissociation and perform calculations using Ka and Kb. Calculate the equilibrium concentrations, pH and/or pOH of various species using initial concentrations and the equilibrium constant. (ICE problems) 5) Acid/Base Titrations (5 hours) Titrations are used to reinforce empirically, the rationale of why acids and bases behave as they do. Interpret a variety of titration curves with weak and strong, acids and bases and with mono and polyprotic acids. Select the appropriate indicator for various titrations. Use titration curves or data to predict the pH of various household substances. 214-1, 320-1, 115-7, 114-2, 115-7, 114-2, 320-2, 214-7, 114-9, 320-5, 117-2, 118-6, 117-7, 320-3, 320-4, 320-6, 213-8, 213-3, 214-5, 215-6, 212-8, 215-2, 213-9, 320-7, 116-2, 214-4, 212-4
Unit 4: Organic Chemistry (24 hours) 1) So Many Compounds (3 hrs) Students investigate the large number of organic compounds that result from the unique nature of carbon. Students practice building and illustrating some of these compounds. 2) Influences of Organic Chemistry on Society (1 hr) Natural and synthetic compounds are discussed with respect to their influence on society. 3) Classifying Organic Compounds (2 hrs) Compounds are classified into various families by virtue of their functional groups and structures. 4) Naming and Writing Organic Compounds (5 hrs) Students will name limited numbers of alkanes, alkenes, alkynes, aromatics, alkyl halides, alcohols, carboxylic acids, esters, ethers, aldehydes and ketones. Naming is demonstrated using IUPAC rules. 5) Isomers in Organic Chemistry (2 hrs) Students will illustrate and name structural and geometric isomers of various organic compounds. 319-4, 116-7, 115-3, 115-6,115-1, 319-7, 319-5, 214-2, 319-6, 214-11, 117-5, 114-4, 118-4, 214-9, 319-8, 319-9, 212-2, 212-3, 213-8, 215-1,116-6, 118-2, 215-5, 213-7, 215-3, 117-4
Applications of Organic Chemistry (2 hrs) 6)Students investigate how science and technology contributes to the production of more commercially viable products. An appropriate example of this is oil refining with its incorporation of fractional distillation, cracking and reforming. 7) Writing and Balancing Equations (4 hrs) Complete, balance and classify selected organic reactions. Draw the structural diagrams of all the reactants and products. Include addition, substitution, esterification, 8) Polymerization (1 hr) The process of polymerization is described (addition and condensation) and some important natural and synthetic polymers are identified. 9) Organic Experimentation (2 hrs) Design and perform an experiment. Students could synthesize an ester, aspirin, nylon,… 10) Risk and Benefit of Organic Chemistry: STSE Perspectives (2 hrs) Students could research the risks and benefits of various synthesized organic compounds. (Cfc’s, PCB’s, DDT, BPA,)
CHEM 121
Outcomes
Essential Questions
Unit 1: Organic Chemistry(24 hours) 1) So Many Compounds (3 hrs) Students investigate the large number of organic compounds that result from the unique nature of carbon. Students practice building and illustrating some of these compounds. 2) Influences of Organic Chemistry on Society (1 hr) Natural and synthetic compounds are discussed with respect to their influence on society. 3) Classifying Organic Compounds (2 hrs) Compounds are classified into various families by virtue of their functional groups and structures. 4) Naming and Writing Organic Compounds (5 hrs) Students will name limited numbers of alkanes, alkenes, alkynes, aromatics, alkyl halides, alcohols, carboxylic acids, esters, ethers, aldehydes and ketones. Naming is demonstrated using IUPAC rules. 5) Isomers in Organic Chemistry (2 hrs) Students will illustrate and name structural and geometric isomers of various organic compounds. 319-4, 116-7, 115-3, 115-6,115-1, 319-7, 319-5, 214-2, 319-6, 214-11, 117-5, 114-4, 118-4, 214-9, 319-8, 319-9, 212-2, 212-3, 213-8, 215-1,116-6, 118-2, 215-5, 213-7, 215-3, 117-4
Applications of Organic Chemistry (2 hrs) 6)Students investigate how science and technology contributes to the production of more commercially viable products. An appropriate example of this is oil refining with its incorporation of fractional distillation, cracking and reforming. 7) Writing and Balancing Equations (4 hrs) Complete, balance and classify selected organic reactions. Draw the structural diagrams of all the reactants and products. Include addition, substitution, esterification, 8) Polymerization (1 hr) The process of polymerization is described (addition and condensation) and some important natural and synthetic polymers are identified. 9) Organic Experimentation (2 hrs) Design and perform an experiment. Students could synthesize an ester, aspirin, nylon,… 10) Risk and Benefit of Organic Chemistry: STSE Perspectives (2 hrs) Students could research the risks and benefits of various synthesized organic compounds. (Cfc’s, PCB’s, DDT, BPA,)
Unit 2: Thermochemistry (23 hours) 1) Introduction to Thermochemistry (4 hrs) The relevance of thermochemistry is introduced with the investigation of calorimetry to analyze food products. Alternative fuel energies are investigated with respect to non fossil-fuel combustion. -Thermochemistry STSE -Science Decisions
2)-Thermochemistry Experimentation 3) Bonding and Hess’ Law (5 hrs) Theoretical enthalpy is calculated using Hess’ law for instances where practical applications cannot be applied. 117-6,118-2, 118-8,118-10, 114-5, 213-6, 213-7, 215-4, 324-2,324-5, 214-3, 324-7, 324-1, 324-3, 215-6,212-8 ,212-3, 324-6, 117-9, 214-15,324-4, 214-6, 116-4
Unit 3: From Solutions to Kinetics to Equilibrium (15 hours) 1) Kinetics and Rate of Reaction (3 hrs) Factors affecting the rates of reaction relating to kinetics are investigated. 2) Collision Theory, Reaction Mechanisms and Catalysts (3 hrs) Collision theory and Le Châtelier’s principle are used in predicting the direction of reactions. 3) Chemical Equilibrium (9 hrs) Calculating equilibrium constants is used in predicting the direction of reactions. 321-3, ACC-1, ACC-2, 213-5 323-3, 213-1, 212-9, 323-5, 116-2, 116-4,
Unit 4: Acids and Bases(23 hours) 1) Properties and Definitions of Acids and Bases (4 hrs) Using various models (Arrhenius, and Brønsted-Lowry), students learn the various characteristics, properties and behaviors of acids and bases. The limitations of the Arrhenius Theory are identified. Individual ion concentrations are calculated based on dissociation equations. 2) Acid/Base Reactions (4 hrs) The Brønsted-Lowry Theory is explored in detail. Acids, bases, conjugate acid-base pairs and amphoteric substances are identified. Students learn to predict the products of acid-base reactions by using a table of acid-base strengths. 3) OH-, H3O and Le Châtelier (3 hrs) The self-ionization of water and Kw is introduced. Illustrate the use of indicators and Le Chateliers Principle in action. 4) Using the Equilibrium Concept with Acids and Bases (7 hrs) Perform calculations of pH, pOH, and so on using Kw. Identify strong acids and bases. Identify weak acids and bases, define % dissociation and perform calculations using Ka and Kb. Calculate the equilibrium concentrations, pH and/or pOH of various species using initial concentrations and the equilibrium constant. (ICE problems) .
5) Acid/Base Titrations (5 hours) Titrations are used to reinforce empirically, the rationale of why acids and bases behave as they do. Interpret a variety of titration curves with weak and strong, acids and bases and with mono and polyprotic acids. Select the appropriate indicator for various titrations Use titration curves or data to predict the pH of various household substances. 214-1, 320-1, 115-7, 114-2, 115-7, 114-2, 320-2, 214-7, 114-9, 320-5, 117-2, 118-6, 117-7, 320-3, 320-4, 320-6, 213-8, 213-3, 214-5, 215-6, 212-8, 215-2, 213-9, 320-7, 116-2, 214-4, 212-4
NB Prescribed Outcomes
describe the importance of peer review in the development of your knowledge about thermochemistry. (114-5)
use library and electronic research tools to collect information on a given topic. (213-6)
select and integrate information from various print and electronic sources or from several parts of the same source. (213-7)
identify multiple perspectives that influence a science-related decision or issue involving thermochemistry. (215-4)
define endothermic reaction, exothermic reaction, specific heat capacity, enthalpy, bond energy, heat of reaction, and molar enthalpy. (324-2)
define thermochemistry and thermodynamics.
differentiate between endothermic and exothermic changes.
calculate specific heat capacity.
use specific heat capacity in calculations.
perform heat transfer problem
illustrate changes in energy of various chemical reactions, using potential energy diagrams. (324-5)
dentify exothermic and endothermic processes from the sign of Δ, from thermochemical equations, and from labeled enthalpy/ potential energy diagrams.
label enthalpy diagrams given either the Δ for a process or a thermochemical equation.
compile and display evidence and information on heats of formation in a variety of formats, including diagrams, flow charts, tables, and graphs. (214-3)
write thermochemical equations including the quantity of energy exchanged given either the value of Δ or a labeled enthalpy diagram, and vice versa
compare the molar enthalpies of several combustion reactions involving organic compounds. (324-7)
write and balance chemical equations for combustion reactions of alkanes, including energy amounts. (324-1)
calculate and compare the energy involved in chemical reactions. (324-3)
calculate the changes in energy of various chemical reactions using bond energy, heats of formation, and Hess’s Law (324-4)
apply one of the methods of predicting heats of reactions to your experimentally determined lab values (214-6)
-
conduct a Hess’s Law experiment
compare experimental results to theoretical calculations from heat of formation or bond energy data
analyse and describe examples where technologies were developed based on understanding thermochemistry (116-4)
Students will be expected to
work cooperatively with team members to develop and carry out thermochemistry experiments (215-6)
evaluate and select appropriate instruments for collecting evidence and appropriate processes for problem solving and inquiring (212-8)
design a thermochemistry experiment identifying and controlling major variables (212-3)
determine experimentally the changes in energy of various chemical reactions (324-6)
analyse the knowledge and skills acquired in their study of thermochemistry to identify areas of further study related to science and technology (117-9)
-
compare physical, chemical, and nuclear changes in terms of the species and the magnitude of energy changes involved
propose alternative solutions to solving energy problems and identify the potential strengths and weaknesses of each (214-15)
-
explain, in simple terms, the energy changes of bond breaking and bond formatio
write thermochemical equations to represent enthalpy notation, Δcomb , Δfus, Hvap .
calculate the heat gained or lost from a system using the thermochemical equatio
Ch 22, 23 Organic Chemistry
CHEM 122
Outcomes
Essential Questions(23 hours)
1) Introduction to Thermochemistry (4 hrs) The relevance of thermochemistry is introduced with the investigation of calorimetry to analyze food products. Alternative fuel energies are investigated with respect to non fossil-fuel combustion.
-Thermochemistry STSE
-Science Decisions
2) Enthalpy (14 hrs)
Identify and calculate energy changes associated with phase changes. The construction of heat curves and the analysis of its individual components are explored both qualitatively and quantitatively. A lab reinforces this concept through construction of a basic calorimeter. “Heat Capacity of Calorimeter” “Heat of Reaction” “Specific Heat of a Metal”
-Enthalpy Changes
-Thermochemistry Experimentation
3) Bonding and Hess’ Law (5 hrs) Theoretical enthalpy is calculated using Hess’ law for instances where practical applications cannot be applied.
117-6,118-2,
118-8,118-10, 114-5, 213-6, 213-7, 215-4,
324-2,324-5,
214-3, 324-7, 324-1, 324-3, 215-6,212-8
,212-3, 324-6, 117-9, 214-15, 324-4, 214-6, 116-4
(15 hours)
1) Kinetics and Rate of Reaction (3 hrs) Factors affecting the rates of reaction relating to kinetics are investigated.
2) Collision Theory, Reaction Mechanisms and Catalysts (3 hrs) Collision theory and Le Châtelier’s principle are used in predicting the direction of reactions.
3) Chemical Equilibrium (9 hrs) Calculating equilibrium constants is used in predicting the direction of reactions.
321-3, ACC-1,
ACC-2, 213-5
323-3, 213-1,
212-9, 323-5,
116-2, 116-4,
1) Properties and Definitions of Acids and Bases (4 hrs)
Using various models (Arrhenius, and Brønsted-Lowry), students learn the various characteristics, properties and behaviors of acids and bases. The limitations of the Arrhenius Theory are identified. Individual ion concentrations are calculated based on dissociation equations. 2) Acid/Base Reactions (4 hrs) The Brønsted-Lowry Theory is explored in detail. Acids, bases, conjugate acid-base pairs and amphoteric substances are identified. Students learn to predict the products of acid-base reactions by using a table of acid-base strengths. 3) OH-, H3O and Le Châtelier (3 hrs) The self-ionization of water and Kw is introduced. Illustrate the use of indicators and Le Chateliers Principle in action. 4) Using the Equilibrium Concept with Acids and Bases (7 hrs) Perform calculations of pH, pOH, and so on using Kw. Identify strong acids and bases. Identify weak acids and bases, define % dissociation and perform calculations using Ka and Kb. Calculate the equilibrium concentrations, pH and/or pOH of various species using initial concentrations and the equilibrium constant. (ICE problems)
5) Acid/Base Titrations (5 hours) Titrations are used to reinforce empirically, the rationale of why acids and bases behave as they do. Interpret a variety of titration curves with weak and strong, acids and bases and with mono and polyprotic acids. Select the appropriate indicator for various titrations. Use titration curves or data to predict the pH of various household substances.
214-1, 320-1, 115-7, 114-2,
115-7, 114-2, 320-2, 214-7,
114-9, 320-5, 117-2, 118-6,
117-7, 320-3, 320-4, 320-6,
213-8, 213-3, 214-5, 215-6,
212-8, 215-2, 213-9, 320-7,
116-2, 214-4, 212-4
1) So Many Compounds
(3 hrs) Students investigate the large number of organic compounds that result from the unique nature of carbon. Students practice building and illustrating some of these compounds.
2) Influences of Organic Chemistry on Society (1 hr) Natural and synthetic compounds are discussed with respect to their influence on society.
3) Classifying Organic Compounds (2 hrs) Compounds are classified into various families by virtue of their functional groups and structures.
4) Naming and Writing Organic Compounds
(5 hrs)
Students will name limited numbers of alkanes, alkenes, alkynes, aromatics, alkyl halides, alcohols, carboxylic acids, esters, ethers, aldehydes and ketones. Naming is demonstrated using IUPAC rules.
5) Isomers in Organic Chemistry (2 hrs)
Students will illustrate and name structural and geometric isomers of various organic compounds.
319-4, 116-7, 115-3, 115-6,115-1, 319-7,
319-5, 214-2, 319-6, 214-11, 117-5, 114-4,
118-4, 214-9, 319-8, 319-9, 212-2, 212-3,
213-8, 215-1,116-6, 118-2, 215-5, 213-7,
215-3, 117-4
(2 hrs)
6)Students investigate how science and technology contributes to the production of more commercially viable products. An appropriate example of this is oil refining with its incorporation of fractional distillation, cracking and reforming.
7) Writing and Balancing Equations (4 hrs) Complete, balance and classify selected organic reactions. Draw the structural diagrams of all the reactants and products. Include addition, substitution, esterification,
8) Polymerization (1 hr) The process of polymerization is described (addition and condensation) and some important natural and synthetic polymers are identified. 9) Organic Experimentation (2 hrs) Design and perform an experiment. Students could synthesize an ester, aspirin, nylon,…
10) Risk and Benefit of Organic Chemistry: STSE Perspectives (2 hrs) Students could research the risks and benefits of various synthesized organic compounds. (Cfc’s, PCB’s, DDT, BPA,)
CHEM 121
Outcomes
Essential Questions1) So Many Compounds
(3 hrs) Students investigate the large number of organic compounds that result from the unique nature of carbon. Students practice building and illustrating some of these compounds.
2) Influences of Organic Chemistry on Society (1 hr) Natural and synthetic compounds are discussed with respect to their influence on society.
3) Classifying Organic Compounds (2 hrs) Compounds are classified into various families by virtue of their functional groups and structures.
4) Naming and Writing Organic Compounds
(5 hrs)
Students will name limited numbers of alkanes, alkenes, alkynes, aromatics, alkyl halides, alcohols, carboxylic acids, esters, ethers, aldehydes and ketones. Naming is demonstrated using IUPAC rules.
5) Isomers in Organic Chemistry (2 hrs)
Students will illustrate and name structural and geometric isomers of various organic compounds.
319-4, 116-7, 115-3, 115-6,115-1, 319-7,
319-5, 214-2, 319-6, 214-11, 117-5, 114-4,
118-4, 214-9, 319-8, 319-9, 212-2, 212-3,
213-8, 215-1,116-6, 118-2, 215-5, 213-7,
215-3, 117-4
(2 hrs)
6)Students investigate how science and technology contributes to the production of more commercially viable products. An appropriate example of this is oil refining with its incorporation of fractional distillation, cracking and reforming.
7) Writing and Balancing Equations (4 hrs) Complete, balance and classify selected organic reactions. Draw the structural diagrams of all the reactants and products. Include addition, substitution, esterification,
8) Polymerization (1 hr) The process of polymerization is described (addition and condensation) and some important natural and synthetic polymers are identified. 9) Organic Experimentation (2 hrs) Design and perform an experiment. Students could synthesize an ester, aspirin, nylon,…
10) Risk and Benefit of Organic Chemistry: STSE Perspectives (2 hrs) Students could research the risks and benefits of various synthesized organic compounds. (Cfc’s, PCB’s, DDT, BPA,)
Unit 2: Thermochemistry
(23 hours)
1) Introduction to Thermochemistry (4 hrs) The relevance of thermochemistry is introduced with the investigation of calorimetry to analyze food products. Alternative fuel energies are investigated with respect to non fossil-fuel combustion.
-Thermochemistry STSE
-Science Decisions
3) Bonding and Hess’ Law (5 hrs) Theoretical enthalpy is calculated using Hess’ law for instances where practical applications cannot be applied.
117-6,118-2,
118-8,118-10, 114-5, 213-6, 213-7, 215-4,
324-2,324-5,
214-3, 324-7, 324-1, 324-3, 215-6,212-8
,212-3, 324-6, 117-9, 214-15,324-4, 214-6, 116-4
Unit 3: From Solutions to Kinetics to Equilibrium
(15 hours)
1) Kinetics and Rate of Reaction (3 hrs) Factors affecting the rates of reaction relating to kinetics are investigated.
2) Collision Theory, Reaction Mechanisms and Catalysts (3 hrs) Collision theory and Le Châtelier’s principle are used in predicting the direction of reactions.
3) Chemical Equilibrium (9 hrs) Calculating equilibrium constants is used in predicting the direction of reactions.
321-3, ACC-1,
ACC-2, 213-5
323-3, 213-1,
212-9, 323-5,
116-2, 116-4,
1) Properties and Definitions of Acids and Bases (4 hrs)
Using various models (Arrhenius, and Brønsted-Lowry), students learn the various characteristics, properties and behaviors of acids and bases. The limitations of the Arrhenius Theory are identified. Individual ion concentrations are calculated based on dissociation equations. 2) Acid/Base Reactions (4 hrs) The Brønsted-Lowry Theory is explored in detail. Acids, bases, conjugate acid-base pairs and amphoteric substances are identified. Students learn to predict the products of acid-base reactions by using a table of acid-base strengths. 3) OH-, H3O and Le Châtelier (3 hrs) The self-ionization of water and Kw is introduced. Illustrate the use of indicators and Le Chateliers Principle in action. 4) Using the Equilibrium Concept with Acids and Bases (7 hrs) Perform calculations of pH, pOH, and so on using Kw. Identify strong acids and bases. Identify weak acids and bases, define % dissociation and perform calculations using Ka and Kb. Calculate the equilibrium concentrations, pH and/or pOH of various species using initial concentrations and the equilibrium constant. (ICE problems)
.
(5 hours)
Titrations are used to reinforce empirically, the rationale of why acids and bases behave as they do. Interpret a variety of titration curves with weak and strong, acids and bases and with mono and polyprotic acids. Select the appropriate indicator for various titrations
Use titration curves or data to predict the pH of various household substances.
214-1, 320-1, 115-7, 114-2,
115-7, 114-2, 320-2, 214-7,
114-9, 320-5, 117-2, 118-6,
117-7, 320-3, 320-4, 320-6,
213-8, 213-3, 214-5, 215-6,
212-8, 215-2, 213-9, 320-7,
116-2, 214-4, 212-4